tya Posted March 28, 2011 Share Posted March 28, 2011 i did an experiment on solubility product constant which involves titration of concentrated calcium hydroxide and HCl at constant temperature and we did titration to find the Ksp. but now i can't figure out what is the relationship between reaction of Ca(OH)2 used to neutralised HCl with Ksp definition. does it means that in the calcium hydroxide solution, Ca(OH)2 the sparingly soluble salt is not completely ionised and only the ions are able to react with HCl? also since Ca(OH)2 is used, will the equilibrium of saturated solution be affected (Le Chatelier"s Principle)? Link to comment Share on other sites More sharing options...
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